Question

How many moles of Fe3O4 (used in biomedical nanoparticles) are required to supply enough iron to prepare 0.844 mol Fe2O3? Enter your answer in accordance with the question statement mol Fe3O4

A) 0.422 mol Fe3O4
B) 1.266 mol Fe3O4
C) 2.688 mol Fe3O4
D) 4.022 mol Fe3O4

Answer 1

To determine the number of moles of Fe3O4 required, use the stoichiometry of the reaction. Multiply the number of moles of Fe2O3 by the mole ratio of Fe3O4 to Fe2O3 from the balanced equation.

Step-by-step explanation:

To determine the number of moles of Fe3O4 required to supply enough iron to prepare 0.844 mol Fe2O3, we need to consider the stoichiometry of the reaction. The balanced equation for the reaction is:

2 Fe3O4 + 3 O2 -> 6 Fe2O3

From the balanced equation, we can see that 2 moles of Fe3O4 are required to produce 6 moles of Fe2O3. This means that for every 6 moles of Fe2O3, we need 2 moles of Fe3O4.

Therefore, the number of moles of Fe3O4 required to supply enough iron to prepare 0.844 mol Fe2O3 is:

0.844 mol Fe2O3 * (2 mol Fe3O4 / 6 mol Fe2O3) = 0.281 mol Fe3O4